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Year 12 Take 1 Chem > Unit four JCL > Flashcards

Unit four JCL Flashcards

1
Q

Group 1 metals oxidation state

A

always +1

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2
Q

Group 2 metals oxidation state

A

always +2

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3
Q

Oxygen oxidation state

A

usually -2 (except in peroxides, where it is -1 and F2O, where it is +2)

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4
Q

Hydrogen oxidation state

A

usually +1 (except in metal hydrides, where it is -1)

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5
Q

Fluorine oxidation state

A

always -1

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6
Q

Chlorine oxidation state

A

usually -1 (except in compounds with O or F)

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7
Q

What increases as you go down group 2

A

Reactivity, Atomic Radius, Reaction with water, Solubility of Hydroxide

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8
Q

What decreases as you go down group 2

A

1st ionization energy, Melting point, Solubility of Sulfate

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9
Q

What are oxidizing agents

A

They cause anther species to be oxidized by taking electrons, The oxidizing agents themselves are reduced

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10
Q

What is a displacement reaction

A

A reaction in which a more reactive element displaces a less reactive element from an aqueous solution of its ion

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11
Q

What colour is the water and cyclohexane for Cl2

A

water: pale-green
cyclohexane: pale-green

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12
Q

What colour is the water and cyclohexane for Br2

A

water: Orange
cyclohexane: Orange

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13
Q

What colour is the water and cyclohexane for I2

A

water: Brown
cyclohexane: Violet

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14
Q

What is a disproportionation reaction

A

A redox reaction in which the same element is both oxidised and reduced

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15
Q

Identifying halide ions, precipitate colour

A

AgCl: white
AgBr: cream
AgI: yellow

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16
Q

Identifying halide ions, solubility of silver halide solution in NH3

A

AgCl: soluble in dilute NH3 (ammonia)
AgBr: soluble in concentrated NH3
AgI: insoluble in concentrated NH3

17
Q

What is the trend in oxidising power down group seven?

A

It decreases

18
Q

Test for carbonate ion?

A

Put in dilute acid, bubble through lime water, turns cloudy

19
Q

Test for sulphate ion?

A

Add barium chloride, forms white precipitate

20
Q

Test for ammonium ion?

A

Add sodium hydroxide and heat, red litmus paper will turn blue from ammonia gas produced

21
Q

Define first ionization energy

A

The first ionization energy of an element is the energy required to remove one electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions

22
Q

Define successive ionisation energy

A

Successive ionization energies of an element are a measure of the energy required to remove each electron in turn

23
Q

How does electron shielding effect ionization energy?

A

More inner shell electrons –> greater distance –> less nuclear attraction on outer shell electrons

24
Q

How does atomic radius effect ionization energy?

A

Greater radius –> less nuclear attraction on outer shell electrons

25
Q

How does nuclear charge effect ionization energy?

A

Greater nuclear charge –> greater attractive force on the outer shell electrons

26
Q

Why is there a drop in first ionization energy between p and s?

A

The electrons are in a new sub-shell that is higher in energy so it takes less energy to remove an electron

27
Q

Why is sodium described as an s-block element?

A

Its outermost electron is in the s sub-shell

28
Q

What is metallic bonding?

A

The electrostatic attraction between po0sitive metal ions and delocalized electrons

29
Q

What does delocalized mean?

A

Electrons are free to move and are not fixed to one specific ion/atom

30
Q

What does the word lattice mean?

A

A regularly repeating pattern

31
Q

What is a giant metallic lattice?

A

A 3D structure of regularly arranged positive ions in a sea of delocalized electrons bonded by strong metallic bonds

32
Q

Melting/ boiling point in metals

A

High melting and boiling points

33
Q

Electrical conductivity in metals

A

Good conductivity

34
Q

Physical manoeuvability

A

Malleable and ductile

35
Q

Malleable definition

A

Can be hammered into shape

36
Q

Ductile definition

A

Can be drawn out into wires

37
Q

Why do metals have high melting and boiling points

A

Strong electrostatic attraction between positive metal ions and negative electrons, metallic bonds require high amounts of energy to break apart

38
Q

Why are metals good conducters

A

Delocalized electrons are free to move across the metallic lattice and can carry a charge in a uniform direction producing a current

39
Q

Why are metals malleable and ductile?

A

Delocalized electrons can move and layers in the giant metallic lattice are able to slide over each over

Year 12 Take 1 Chem (9 decks)

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